Engineering
Chemistry
Integrated Rate Law
Question

Reaction A + B → C + D follow's following rate law :

rate =k=[A]+12[B]12 .

Starting with initial concentration of one mol of A and B each, what is the time taken for amount of A of become 0.25 mol. Given k = 2.31 × 10–3 sec–1.

600 sec

300 sec

None of these

900 sec

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Solution

A +  B      →    C    +     D
t = 0       1     1        
   ‘t’        1-x    1-x           x         x
rate = k[A]½ [B]½

−d[A]dt=k(1−x)1/2(1−x)1/2⇒−d(1−x)dt=k(1−x)⇒dxdt=k(1−x)

⇒∫0xdx1−x=k∫0tdt ⇒[−1(1−x)]0x=kt ⇒−ln(1−x)=kt

⇒−ln(1−x)=kt ⇒t=1kln(11−x)

When [A] = 0.25
∴  x = 0.75

∴t=12.31×10−3ln10.25=1032.31ln4=2×103×0.6932.31=2×103×0.6932.31=600 Sec.